Transcript Brief history of the atom

Modern Physics vs Classical Physics
MODERN PHYSICS
Electrons
J.J. Thompson
Robert Millikan
Photons
Max Planck
Albert Einstein
Photoelectric Effect
Experiment
The Graph
Energy Levels
Absorption/Emission Spectra
Bohr Model
De Broglie Wavelength
X-Ray Production
Compton Scattering
Nuclear Notation
Energy-Mass Equivalence
Nuclear Decay
Fission
Fusion
The Electron in Brief
We will mainly deal with Electrons and Photons in this unit. Therefore,
We will start with some properties of each particle.
1897: J.J. Thomson Discovered the electron and measured the properties of the
particle (the electron). However, his instruments were crude. He could only measure
the charge to mass ratio, and not the charge or mass itself.
J.J. Thomson’s Experiment
J.J. Thomson’s Experiment
In the year 1896 he led the experiment by which he defined the connection of
particles charge and its mass (q/m). He turned the cathode ray’s beam on the
collector. The beam transferred its charge to the collector and warmed it. He knew
collector's mass, its specific heat and the heat gain. Basing on it he could
evaluated thermal energy. He measured the temperature of the collector using
the light thermosteam fastened to the collector. He measured the total charge
gathered on the collector using very sensitive electrometer.
He obtained a value of ~ q/m = 1*1011 coulombs per kilogram.
Today, the accepted value is 1.768 x1011 coulombs per kilogram
The Electron in Brief
We will mainly deal with Electrons and Photons in this unit. Therefore,
We will start with some properties of each particle.
1897: J.J. Thomson Discovered the electron and measured the properties of the
particle (the electron). However, his instruments were crude. He could only measure
the charge to mass ratio, and not the charge or mass itself.
1906: Robert Millikan devised an experiment to measure the charge of the
electron ( q = -1.6x10-19 C).
This experiment is the famous “Millikan Oil Drop Experiment”
Millikan Oil Drop Experiment
An atomizer sprayed a fine mist of oil droplets into the upper chamber. Some of these
tiny droplets fell through a hole in the upper floor into the lower chamber of the
apparatus. Millikan first let them fall until they reached terminal velocity due to air
resistance. Using the microscope, he measured their terminal velocity and calculated
the mass of each oil drop.
Millikan Oil Drop Experiment
Next, Millikan applied a charge to the falling drops by irradiating the bottom chamber
with x-rays. This caused the air to become ionized, which basically means that the air
particles lost electrons. A part of the oil droplets captured one or more of those extra
electrons and became negatively charged.
By attaching a battery to the plates of the lower chamber he created an electric field
between the plates that would act on the charged oil drops; he adjusted the voltage till
the electric field force would just balance the force of gravity on a drop, and the drop
would hang suspended in mid-air. Some drops have captured more electrons than
others, so they will require a higher electrical field to stop.
Millikan Oil Drop Experiment
Particles that did not capture any of that extra electrons were not affected by the
electrical field and fell to the bottom plate due to gravity.
When a drop is suspended, its weight m · g is exactly equal to the electric force
applied, the product of the electric field and the charge q · E.
The values of E (the applied electric field), m (the mass of a drop which was already
calculated by Millikan), and g (the acceleration due to gravity), are all known values. So
it is very easy to obtain the value of q, the charge on the drop, by using the simple
formula:
m·g=q·E
Millikan Oil Drop Experiment
The Electron in Brief
We will mainly deal with Electrons and Photons in this unit. Therefore,
We will start with some properties of each particle.
1897: J.J. Thompson Discovered the electron and measured the properties of the
particle (the electron). However, his instruments were crude. He could only measure
the charge to mass ratio, and not the charge or mass itself.
1906: Robert Millikan devised an experiment to measure the charge of the
electron ( q = -1.6x10-19 C).
This experiment is the famous “Millikan Oil Drop Experiment”
With Thompson’s charge to mass ratio, and Millikan’s charge, the mass of the electron
could then be calculated: 9.11x10-31 kg
The Photon
blackbody radiation
In the last quarter of the 1800’s scientists had been working on a way
to take what they knew about mechanics, thermodynamics,
electricity & magnetism and optics to describe how hot objects cool
by giving off light in various parts of the electromagnetic spectrum.
The study of this effect is known as blackbody radiation.
You have seen blackbody radiation. Any object
That is hot enough gives off light (blackbody radiation)
The Photon
blackbody radiation
You have seen blackbody radiation. Any object
that is hot enough gives off light (blackbody radiation)
The Photon
blackbody radiation
If an object is hotter than its surroundings it will cool by giving off light. In
order to study this effect scientist had to eliminate the other modes of
cooling. Blocks of graphite were hollowed and a small hole was drilled into
the carbon. Although the outside of the carbon block would cool by
convection as well as radiation, the inside would cool by mostly radiation
alone. The intensity of each wavelength of light emitted by the inside of
the hot, black boxes was studied, hence the name- blackbody radiation.
blackbody radiation
James Clark Maxwell had discovered the equations that governed the production
and transmission of these waves through space and time.
A serious problem arose when the electromagnetic spectrum emitted by a
radiating body did not match the spectrum that should be produced from the
mathematical model of light. The fact that the classical theory did not match the
actual spectrum emitted by objects came to be known as the ultra-violet
catastrophe.
blackbody radiation
1900: Max Planck developed a mathematical model that fit the data without using
any known theory. The idea was to find what function worked and then determine
what the theory would be. Much to the surprise of Planck, the mathematical
model that worked called for light to be jumping off the hot objects in bits and
pieces like particles instead of waves.
blackbody radiation
Energy of a photon:
E = hf
E: the energy
f: the frequency of light
h: a constant (Planck’s Constant) 6.63x10-34 j s
Since Planck’s constant is so small, another way to express
It is in terms of the electronvolt (eV).
1 eV is equal to the amount of kinetic energy gained by a single electron
when it accelerates through an electric potential difference of one volt.
Thus it is 1 volt (1 j/C) multiplied by the electron charge (1.6×10−19 C).
Therefore, one electron volt is equal to 1.6×10−19 J
h: Planck’s constant = 6.63x10-34 j s = 4.14x10-15 eV s
Enter Einstein:
1905: Albert Einstein, while working on his theory of relativity, discovered a
few more properties of light.
1. Photons travel at v = c in a vacuum. c = 3x108 m/s
2. Although photons are particles, photons have no rest mass
(rest mass is the mass of a stationary object)
(no rest mass is unique to photons, everything else has a mass)
3. Although photons do not have mass, they have momentum:
p=h/
(p = h /  only applies to photons, for all other objects, use p = mv)
Enter Einstein:
Momentum of a photon:
p=h/
By substituting: E = hf and c = f  , --> E = hc/  --> E = pc
Therefore, the energy of a photon can be written as:
E = hf
E = hc/ 
E = pc
The product of Planck’s constant and the speed of light show up so
often that the AP exam will have a value listed in the constants table
Example Problem
A 3-milliwatt pen laser radiates at 633 nm. Find values for the
following:
a) Frequency of light emitted
b) energy of a single photon in joules,
c) energy of a photon in electron volts
d) momentum of a single photon.
Example Problem
A 3-milliwatt pen laser radiates at 633 nm. Find values for the
following:
a) Frequency of light emitted, b) energy of a single photon in joules,
c) energy of a photon in electron volts, and d) momentum of a single
photon
a) c = f or
f = c/ = 3x108m/s / 633x10-9 m
f = 4.74x1014 Hz
b) E = hf = 6.63x10-34 Jsec (4.74x1014 1/s)
E = 3.14x10-19 J
c) E = hf = 4.14x10-15 eVs (4.74x1014 1/s)
E = 1.96 eV
d) p = h/ = 6.63x10-34 Jsec/ 6.33x10-9 m
or p = E/c = 3.14x10-19 J / 3x108m/s
p = 1.05x10-27 Nsec
The Photoelectric Effect
Late 1800’s: Heinrich Hertz noticed that under the right conditions
UV light could cause sparks to fly from metal surfaces.
This phenomenon was labeled the
photoelectric effect.
photoelectric effect - The emission of
electrons from material as a result of light
falling on it
What did not make sense about the phenomena was that only light above a
certain threshold frequency would cause the electrons to be ejected from
the surface. Light below that frequency, regardless of its brightness would
not knock electrons off the surface.
The Photoelectric Effect
Principle observations
1. Electrons are emitted only when the frequency of light is above
the threshold value, no matter how intense the light is.
2. Using a setup similar to the one shown below, they found that the KE
of the ejected electrons is directly proportional to the frequency of the
light hitting the metal surface.
3. It was also discovered that the current in the circuit is
proportional to the brightness of the light hitting the metal, but
only if the threshold frequency of the metal was exceeded.
The Photoelectric Effect
Albert Einstein’s Explanation:
In 1905 Albert Einstein gave a very simple explanation of the photoelectric effect
Light is acting like particles. Each electron can absorb a single
photon. When you increase the intensity of light more photons
are created and liberate more electrons. This explains the liner
relationship between the intensity of the light source and the
photocurrent.
The Photoelectric Effect
Albert Einstein’s Explanation:
The Photoelectric Effect
Albert Einstein’s Explanation:
Einstein’s idea incorporated Planck’s quantum hypothesis into a
statement of energy conservation:
The energy (hf) of the photon must be equal to the energy
needed to free the electron plus the electron's KE
KEmax = hf – ф
Ф: the Work Function: the energy needed to free
the electron.
hf: the total energy of the photon.
The Photoelectric Effect
Albert Einstein’s Explanation:
KEmax = hf – ф
The minimum energy (the threshold energy required to
remove an electron from the surface is easy to calculate,
set KE = 0. Therefore,
hfth = ф
This equation is often solved to find the threshold or cutoff frequency
The Photoelectric Effect
Albert Einstein’s Explanation:
Einstein predicted that every metal should produce a linear graph of
the stopping voltage as a function of frequency. And that all of the
graphs should have the same slope.
The equation for the line is:
Y = mx + b
Remember:
KEmax = hf – ф
The Photoelectric Effect
Albert Einstein’s Explanation:
Slope = h
(planck’s constant )
X-intercept = fth (threshold frequency)
Y-intercept = -ф
(work function)
Compton Scattering (Verification that Photons have momentum)
1920’s: Arthur Compton discovered that a photon loses energy
when it collides with an object (electron).
The momentum was transferred, not as a wave, but just like Billiard balls
colliding with each other. The photons were behaving like particles.
The photon’s obey the law of conservation of momentum, just like a particle
with mass.
Compton Scattering
The particle with mass gains energy and momentum during the
collision and the scattered photon loses energy and momentum.
Photons can be scattered in any direction after the collision. The
shift in wavelength is dependant on the angle of scattering. The
bigger the angle, the greater the loss of energy of the photon.
Compton Scattering
Classical mechanics:
m1v1i + m2v2i = m1v1f + m2v2f
Compton Scattering
Classical mechanics:
m1v1i + m2v2i = m1v1f + m2v2f
Compton Scattering
Classical mechanics:
m1v1i + m2v2i = m1v1f + m2v2f
Momentum of a photon: p = h/λ
The set up of the problems are the
same as classical mechanics. You just
have to use the different momentum
equations. Remember, if the particles
deflect at angles, you need to break
them into the X and Y components.
Momentum of an electron: p = mv γ
Implications of wave/particle duality on the Atom
Brief history of the atom
So far we showed that many aspects of light can only be predicted if
we assume light is a particle. Yet it also acts as a wave
(diffraction/interference).
This is called the Wave/Particle duality of light. It is both a wave and
a particle – or something else that we can only measure as a wave or particle.
If light can behave as a particle, can a particle behave as a wave?
Yes
The atom can only be fully explained if we assume it is a wave…
Brief history of the atom
Implications of wave/particle duality on the Atom
Brief history of the atom
J.J. Thomson – Plum Pudding Model:
Plum Pudding does not contain plums!!!
In the 17th century, “plum” referred to raisins and other dried fruits.
Implications of wave/particle duality on the Atom
Brief history of the atom
1904: J.J. Thomson – Plum Pudding Model:
Based on his discovery of the (-) electron, he hypothesized that
the electrons were evenly distributed in a positive substance.
(Electrons were the raisins, the pudding was the positive charge)
The nucleus had not been discovered yet
Implications of wave/particle duality on the Atom
Brief history of the atom
Ernest Rutherford – Electron Orbit Model:
1911: Rutherford conducted a “Gold Foil” Experiment, where he shot
alpha particles through a thin foil of Gold.
Almost all of the particles went straight through the gold. However, some
were deflected.
Based on this information, he concluded that the atom was mostly empty
space. Therefore, the mass of the atom was contained mostly in a tiny
nucleus, and electrons orbited the nucleus like planets orbiting the sun.
Implications of wave/particle duality on the Atom
Brief history of the atom
Ernest Rutherford – Electron Orbit Model:
Implications of wave/particle duality on the Atom
Brief history of the atom
Ernest Rutherford – Electron Orbit Model:
1911: Rutherford conducted a “Gold Foil” Experiment, where he shot
alpha particles through a thin foil of Gold.
Almost all of the particles went straight through the gold. However, some
were deflected.
Based on this information, he concluded that the atom was mostly empty
space. Therefore, the mass of the atom was contained mostly in a tiny
nucleus, and electrons orbited the nucleus like planets orbiting the sun.
Implications of wave/particle duality on the Atom
Brief history of the atom
Ernest Rutherford’s model did not work!
The electrons would slowly spiral into the nucleus every time they gave
off energy.
Implications of wave/particle duality on the Atom
Brief history of the atom
Before we go to the next model, we must understand Spectral lines.
Spectroscopy: The study of spectra which results in
diffracting light into its component colors
Spectra is thought of as the fingerprint
of matter. Each element has it’s own
unique spectrum.
Implications of wave/particle duality on the Atom
Brief history of the atom
Spectroscopy plays a major role in determining the chemical
composition of substances. Most of modern chemistry and
astronomy depends on spectroscopic analysis of materials.
MR spectroscopy of a region
of the brain to detect a tumor
Spectroscopic data of a galaxy to
determine its composition
Implications of wave/particle duality on the Atom
Brief history of the atom
There are two types of Spectra:
Emission: Series of light lines, each represent a particular wavelength
of light. Caused by electrons giving off energy (dropping down an energy
level).
Absorption: Series of dark lines in a spectrum, each line represents a
particular wavelength of light that is absorbed. Caused by electrons
accepting energy (moving up an energy level).
Implications of wave/particle duality on the Atom
Brief history of the atom
Absorption spectra of the Sun:
Implications of wave/particle duality on the Atom
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Emission and Absorption spectrum
Implications of wave/particle duality on the Atom
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Spectroscopy:
Physicists could use spectroscopy to determine compositions,
temperatures, velocities, etc… of many different object. Charts were
made of the spectra of each element.
However, no one could determine the exact cause of the spectral lines.
According to Rutherford’s model, electrons that gave off continuous
energy would spiral into the nucleus of the atom. Another model of the
atom had to be made.
Implications of wave/particle duality on the Atom
Brief history of the atom
Neils Bohr– Energy Level Model:
1913: In order to explain line Spectra, Bohr modified Rutherford's model
by saying electrons can only have special orbits, and electrons can only
jump between these certain orbits (energy levels). In order to jump
between orbits, electrons could only accept or give off discrete “quanta”
of energy (quantum leaps).
Implications of wave/particle duality on the Atom
Brief history of the atom
Neil's Bohr– Energy Level Model:
1913: In order to explain line Spectra, Bohr modified Rutherford's model
by saying electrons can only have special orbits, and electrons can only
jump between these certain orbits (energy levels). In order to jump
between orbits, electrons could only accept or give off discrete “quanta”
of energy (quantum leaps).
Implications of wave/particle duality on the Atom
Brief history of the atom
Implications of wave/particle duality on the Atom
Brief history of the atom
Implications of wave/particle duality on the Atom
Brief history of the atom
Implications of wave/particle duality on the Atom
Brief history of the atom
Energy levels of Bohr’s model of the H atom
Implications of wave/particle duality on the Atom
Brief history of the atom
Energy levels of Bohr’s model of the H atom
Energy =>
hf = Ei - Ef
Implications of wave/particle duality on the Atom
Brief history of the atom
Energy levels of Bohr’s model of the H atom
When using this equation E is the energy from
Bohr’s Energy level diagram.
Make sure E is converted into Joules
Implications of wave/particle duality on the Atom
Brief history of the atom
Problem with Bohr’s model:
Implications of wave/particle duality on the Atom
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Problem with Bohr’s model:
It only works for Hydrogen, or Ionized Helium
(Helium with only 1 electron)
His model does not work for any atom with
more than 1 electron
Implications of wave/particle duality on the Atom
Brief history of the atom
Problem with Bohr’s model:
It only works for Hydrogen, or Ionized Helium
(Helium with only 1 electron)
His model does not work for any atom with
more than 1 electron
So why is his model important? He has
the correct concept (Energy levels).
This led the way into a more correct
model of the Atom.
Implications of wave/particle duality on the Atom
Brief history of the atom
Implications of wave/particle duality on the Atom
Brief history of the atom
Energy levels of the H atom
Implications of wave/particle duality on the Atom
Brief history of the atom
Problem with Bohr’s model:
It only works for Hydrogen, or Ionized Helium
(Helium with only 1 electron)
His model does not work for any atom with
more than 1 electron
So why is his model important? He has
the correct concept (Energy levels).
This led the way into a more correct
model of the Atom.
Implications of wave/particle duality on the Atom
Brief history of the atom
The DeBroglie Hypothesis
In 1924 Louis DeBroglie used the concepts of energy levels from Bohr’s
Incorrect atomic model.
He extended the idea of wave-particle duality to matter, and said all matter
has wave like properties.
h = pλ
 wavelength of a particle
His model turned the electron into a wave. It states that a whole number of
wavelengths must fit into the orbital in order for the orbital to be valid. (This
means each electron wave has to be in a discrete energy level).
Implications of wave/particle duality on the Atom
Brief history of the atom
The DeBroglie Hypothesis
h = pλ
 wavelength of a particle
Not long after DeBroglie’s Hypothesis, Davisson and Germer conducted
an experiment to confirm the wave nature of matter.
Implications of wave/particle duality on the Atom
Brief history of the atom
The DeBroglie Hypothesis
h = pλ
 wavelength of a particle
If all matter has a wavelength, why don’t humans diffract when they walk
through a doorway?
Implications of wave/particle duality on the Atom
Brief history of the atom
The DeBroglie Hypothesis
Not long after DeBroglie’s Hypothesis, Davisson and Germer conducted
an experiment to confirm the wave nature of matter.
Implications of wave/particle duality on the Atom
Brief history of the atom
Heisenberg added to the model by saying since the electron is the entire
standing wave, we cannot pinpoint the electrons exact position. It
occupies the entire wave. (This is “Heisenberg’s uncertainty principle”)
Implications of wave/particle duality on the Atom
Brief history of the atom
Soon Schrodinger and Born added to DeBroglie’s hypothesis. After
Schrodinger and Born, the electron wave model could predict any
energy jump of any atom on the Periodic table (s,p,d,f orbitals)
Implications of wave/particle duality on the Atom
Brief history of the atom
Physicists modern view of atoms
Implications of wave/particle duality on the Atom
Brief history of the atom
Each orbital is a different
wave harmonic where
constructive interference occurs.
The electron is not in
the energy cloud, it is
the energy cloud.
Soon Schrodinger and Born added to DeBroglie’s hypothesis. After
Schrodinger and Born, the electron wave model could predict any
energy jump of any atom on the Periodic table (s,p,d, and f orbitals)
The Atom as a wave
What do atoms look like when viewed through scanning tunneling
microscopes?
The Atom as a wave
What do atoms look like when viewed through scanning tunneling
microscopes?
Waves!
Actual image from a STM. This is an Ag atom. The constructive interference peak
is the nucleus, the diffraction pattern around the peak are the electrons.
The Atom as a wave
What do atoms look like when viewed through scanning tunneling
microscopes?
Waves!
Actual image from a STM. This is a copper surface with two non-copper atoms
creating an electron diffraction pattern. The electrons are the waves. The impure
atoms are the destructive interference troughs.
The Atom as a wave
What do atoms look like when viewed through scanning tunneling
microscopes?
Waves!
Actual image from a STM. This is a ring of 48 iron atoms. The wavelike crests and
Troughs are the electrons. The constructive interference peaks are the iron nuclei
The Atom as a wave
What do atoms look like when viewed through scanning tunneling
microscopes?
Waves!
Actual image from a STM. This is a another ring of 8 iron atoms. The ring creates a
trap for the electrons, and sets up a standing wave pattern in the ring. These
standing waves are the electrons.
The Atom as a wave
What do atoms look like when viewed through scanning tunneling
microscopes?
Waves!
Actual image from a STM. This is another ring of metal atoms with two different
atoms in the centers. Gain, the wave patterns are the electrons.
Implications of wave/particle duality on the Atom
Brief history of the atom
Applications of Quantum Mechanics:
When physicists started thinking of the electron (as well as P+ and N) as a
wave and not a particle, many breakthroughs were made and new
technologies still continue to be developed.
Applications of Quantum Mechanics:
Tunneling
An electron wave has a probability of taking up a certain amount of space.
If it were near a barrier, there is a small chance it will be on the other side of the
barrier.
Applications of Quantum Mechanics:
Tunneling
An electron wave has a probability of taking up a certain amount of space.
If it were near a barrier, there is a small chance it will be on the other side of the
barrier.
Barrier
Electron wave function
(probability cloud)
Applications of Quantum Mechanics:
Tunneling
If the wave function is calculated, and there is a probability of 5% of the electrons
on the other side of the barrier, this means, 5% of the electrons will actually
be on the other side of the barrier.
Barrier
Electron wave function
Applications of Quantum Mechanics:
Tunneling
This is an easy way to control the flow of current in a circuit. A semiconductor uses
The quantum properties of tunneling. Semiconductors are a vital part of almost
any circuitry
Barrier
Electron wave function
Applications of Quantum Mechanics:
Tunneling
Applications of Quantum Mechanics:
Tunneling
After semiconductors were invented, the computer revolution started.
Without semiconductors, there would be no computers and very few other
electronic devices.
(Semiconductors used in circuits include diodes, transistors, and microchips – which are made of transistors)
Standard “key hole” transistors
Model of the 1st transistor, built in 1947
New “Surface Mount” transistors are the size of a grains of sand.
Transistors integrated into chips are currently in the size range of nanometers,
soon they will be in the size range of atoms.
Applications of Quantum Mechanics:
Tunneling
The standard personal computer now has approximately 100 million transistors
High end computers have approximately 1 billion transistors
Approximately every 18 months, the number of transistors in a computer doubles
This microchip performs
computations using 1,000’s of
transistors
Applications of Quantum Mechanics:
Quantum Entanglement
Developed by Einstein, Podolsky, and Rosen in 1935. It’s now called the
EPR paradox.
Einstein refused to believe it calling it “spooky action at a distance” and
insisting it was caused by an error in his math.
Finally, in 1980, Alain Aspect experimentally verified quantum entanglement.
Applications of Quantum Mechanics:
Quantum Entanglement
What is quantum entanglement?
In the press it is often called quantum teleportation. However that is very
misleading.
If a particle is created in a pair, such as two photons emitted by a single
source, the quantum properties of the photons are somehow linked so that
one always knows what the other is doing. When an aspect of one photon’s
quantum state is measured, the other photon instantly changes in response,
even when the two photons are separated by large distances.
Applications of Quantum Mechanics:
Quantum Entanglement
What is quantum entanglement?
Explanation for dummies:
You have two crayons out of a box, one red and one blue. You don’t look at
the crayons and mail a random one to Alaska.
The person you mailed it to wants a blue crayon, you can measure your
crayon at home and say it’s red, This will instantly cause the persons crayon
in Alaska to turn blue.
If the person in Alaska wanted a blue crayon, you can measure your crayon
at home and say it’s blue, the persons crayon in Alaska will instantly turn red.
As soon as you measure the color of your crayon, the color of the Alaska
crayon will instantly turn the opposite color. However, you can choose the
color of your crayon by the type of measurement made, thereby instantly
changing the color of the Alaska crayon to whichever color you want.
(Action at a distance)
Applications of Quantum Mechanics:
Quantum Entanglement
What is quantum entanglement?
Why does this happen?
Applications of Quantum Mechanics:
Quantum Entanglement
What is quantum entanglement?
Why does this happen?
We don’t know!
Quantum mechanics just says it DOES happen and it’s been experimentally
verified.
Applications of Quantum Mechanics:
Quantum Entanglement
Applications of Quantum Mechanics:
Quantum Entanglement
Quantum Entanglement, Wave Superposition, and Quantum vacuum
fluxuations are the principles behind the development of quantum computers.
Quantum computers are currently in their infancy. They were theorized in
1981 (after quantum entanglement was verified in 1980), and are still being
developed . A quantum computer will be able to perform calculations using
virtually no processing power in virtually no time. They will be 10,000’s of
times faster and much smaller than today's computers.
Today's computers use “bits of data…megabytes, gigabytes, etc…Each bit
has a value of 1 or 0.
Quantum computers use the superposition of wave functions “qubits” instead
of bits. Each wave function can be1 or 0 or both at the same time
(superposition of the wave function).
Applications of Quantum Mechanics:
Quantum Entanglement
Quantum Entanglement, Wave Superposition, and Quantum vacuum
fluxuations are the principles behind the development of quantum computers.
Since a “qubit” can have all values, Calculations can be performed without
actually running the calculations. Each photon or electron can occupy
multiple places simultaneously (wave nature), However, it can only make an
actual appearance at one location. Its presence defines its path, and that
can, in a very strange way, negate the need for the algorithm (calculation) to
run.
In a nutshell: the photons or electron states that never existed can perform
the calculations, and because of entanglement, the real photon or electron
will have the answer (state = 1 or 0).
A quantum computer can solve a problem without ever running the problem.
Therefore, it’s really fast!
Applications of Quantum Mechanics:
Quantum Computers
Applications of Quantum Mechanics:
Quantum Computers
Quantum Mechanics Review: